# Download Tuesday, Define the law of definite proportions

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Transcript
```Chemistry I
February 1st – 5th
Name___________________________
Muhiga Weekly
Moles
Monday, Find molar mass of PCl3
Tuesday, What is the mass of 1.00 mol of sodium hydrogen carbonate?
Wednesday, Find molar mass.
CO2
SF7
Thursday, Calculate the mass, in grams, of 2.50 mol of iron (II) hydroxide.
Chemistry I
February 1st – 5th
Name___________________________
Muhiga Weekly
Moles
Daily Homework:
Monday, Feb 01:
Mole Activity Questions
Tuesday, Feb 02:
Read 10.1 pg. 306-315
Ques. 9-15
Wednesday, Feb 03: Mole-mass
Worksheet
Thursday, Feb 04: Read 10.2 pg
317-323, Ques. 24-32
Friday, Feb 05:
No School
Events this Week:
02/01: Ch 10: The Mole Activity
02/02: Ch 10.2: Mole -Mass
02/03: Ch 10.2: The Mole -Volume
02/04: Ch 10.3: Percent Composition
02/05: No School
State Standards:
C. 4.3: Given mass of a sample, use the mole concept to determine the
number of moles and number of atoms or molecules in samples of elements
and compounds.
C. 4.7: Perform calculations to determine the composition of a compound or
mixture when given the formula
Key-Terms/ Vocabulary: mole, Avogadro’s # representative particles,
molar mass, Avogadro’s hypothesis, standard temperature and pressure
(STP), molar volume, percent composition, empirical formula, molecular
formula.
Objectives:
Check off the objectives once you feel you understand the material
well.
I will be able to:
___: Convert any given amount of substance to the needed quantity.
___: Explain/show how chemists measure and count substances.
___: Determine the molar mass of an element or compound.
___: Use dimensional analysis to convert the mass of a substance to
moles, or moles to mass.
___: Use dimensional analysis to convert the volume of a gas at STP
to the number of moles, or moles to volume at STP
Big Idea This Week
The mole (mol) is a unit used to count particles indirectly. A mole, also called Avogadro’s
number may be expressed as 6.02 x 10 23, gram molecular mass and molar mass of the representative
particles of that substance (atoms, ions, molecules or formula units).
One mole of a gas occupies a volume of 22.4 L at STP (standard temperature and pressure).
Standard pressure is equivalent to 101.3 kPa, 1atm, or 760 mm Hg, while standard temperature is
equivalent to 273 K, 00C or -32 0F.
The molar mass of an element is the numerical equivalent of the atomic mass (amu) in grams.
Subscripts in a chemical formula indicate how many mols of each element are in one mol of the
compound. The molar mass of a compound is the sum of all the masses of the moles of elements
present in the compound
Inter-conversions between moles and other quantities, e.g., grams, particles and liters may be
accomplished using dimensional analysis. In determining the formula of a compound, the relative
amounts of the elements present in the compound should be obtained through measurement. This
information is then expressed as the percent composition.
```
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